ostwald's dilution law

The Ostwald’s Dilution Law is defined for a weak electrolyte as “ the degree of ionization is proportional to the square root of the molar concentration or directly proportional to square root of the volume of the solution which contains one mole of the electrolyte.”

Mathematically, we can write Ostwald’s Dilution Law as below:e

                                           α = √ k_a/C   = √ k_aV

                                     Or, α = √ k_b/C   = √ k_bV

Wilhelm Ostwald’s dilution law is a relationship proposed in 1888 between the dissociation constant Kd and the degree of dissociation α of a weak electrolyte. The law takes the form Where the square brackets denote concentration, and c₀ is the total concentration of electrolyte. Ostwald's dilution law describes the dissociation constant of the weak electrolyte with the degree of dissociation (α) and the concentration of the weak electrolyte.  α = degree of dissociation. Ostwald's dilution law states that only at infinite dilution the weak electrolyte undergoes complete ionization.